Terms/Vocabulary related to Covalent Bonding
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| covalent bonding is the formation of compounds by _?_ electrons between atoms | sharing
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| attraction of atoms for mutually shared electrons is the basis of a ccovalent _?_ | bond
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| abbreviation for most stable arrangement of valence electrons (no periods in abbreviation) | ngc
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| covalent bonding most commonly occurs between 2 _?_ elements | nonmetal
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| a single atom of a noble gas might be described as a _?_ molecule' | monatomic
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| in H:H, the electrons holding the molecule together are called a bonding pair, a covalent electron pair, or simply a _?_ pair | shared
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| in :NH₃, the 2 valence electrons around N that are NOT involved in bonding are called an unshared pair, a nonbonding pair, or simply a _?_ pair | lone
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| the statement "valence electrons rearrange themselves during bonding so that both bonded atoms attain a noble gas configuration" is known as the _?_ rule | octet
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| the mnemonic BrINClHOF identifies the _?_ elements that bond with themselves | diatomic
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| a neutral, stable cluster of covalently-bonded atoms OR the smallest unit of a covalent compound | molecule
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| a _?_ covalent bond consists of 2 electrons, one provided by each bonding atom | single
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| a _?_ covalent bond consists of 4 electrons, two of which are provided by each bonding atom | double
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| a _?_ covalent bond consists of 6 electrons, three of which are provided by each bonding atom | triple
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| diatomic element held together by a double bond | oxygen
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| diatomic element held together by a triple bond | nitrogen
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| shape of any molecule consisting of only two atoms | linear
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| term that describes any compound consisting of only two elements (may be >2 atoms) | binary
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| a _?_ formula shows the arrangement of atoms in space (examples: H–Cl or O=C=O) | structural
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| a _?_ formula tells the # and kinds of atoms in the smallest unit of a covalent compound | molecular
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| shape of a water molecule, H₂O | bent
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| shape of an ammonia molecule, NH₃ | pyramidal
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| shape of a methane molecule, CH₄ | tetrahedral
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| the _?_ theory explains that molecular geometry (shape) is a result of electrons in bonds spreading out to minimize repulsions | VSEPR
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| the _?_ theory explains that atomic orbitals of different energy can rearrange themselves into an equivalent number of molecular orbitals of identical energy (ex: s+p+p+p = 4 sp³'s) | hybridization
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| numerical prefix meaning "1" | mono
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| numerical prefix meaning "2" | di
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| numerical prefix meaning "3" | tri
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| numerical prefix meaning "4" | tetra
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| numerical prefix meaning "5" | penta
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| numerical prefix meaning "6" | hexa
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| numerical prefix meaning "7" | hepta
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| numerical prefix meaning "8" | octa
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| numerical prefix meaning "9" | nona
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| numerical prefix meaning "10" | deca
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| the BF₃ molecule has a trigonal _?_ shape that looks a little like a Mercedes Benz emblem | planar
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| the PCl₅ molecule has a(n) trigonal _?_ shape with a central trigonal planar shape and 2 other bonds vertically above & below that plane | bipyramidal
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| the SF₆ molecule has a(n) _?_ shape consisting of 6 bonds separated by angles of 90º along the x,y,z coordinates | octahedral
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| any naming system (ex: using Roman numerals for ionic, but numerical prefixes for covalent compounds) | nomenclature
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| measure of the attraction of an atom for the electrons in a bond | electronegativity
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| the electronegativity scale ranges from 0.0 to _?_ | 4.0
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| the electronegativity scale is often considered unitless, but recently the _?_ is used to honor the discoverer of this property | pauling
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| a(n) _?_ covalent bond is one in which the electrons are shared equally | nonpolar
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| a(n) _?_ covalent bond is one in which the electrons are shared, but unequally | polar
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| in a(n) _?_ bond, 1 or more electrons are lost by one atom and gained by another | ionic
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| bond classification when the electronegativity difference between the two bonded atoms is 0.0 - 0.4 | nonpolar
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| bond classification when the electronegativity difference between the two bonded atoms is 0.5 - 1.9 | polar
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| bond classification when the electronegativity difference between the two bonded atoms is 2.0 or greater | ionic
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| the weak attractions that hold one molecule to another in solids and liquids are collectively called _?_ (or VDW) forces | intermolecular
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| the weakest intermolecular force caused by random motion of electrons in bonds that leads to a temporary unbalanced distribution and momentary slight areas of charge is called London _?_ or _?_ interaction (same word for both!) | dispersion
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| dipole-dipole forces are moderate intermolecular forces between _?_ molecules | polar
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| the strongest intermolecular force arising from attraction between a hydrogen in a very polar bond and a nearby long pair in another molecule is called _?_ bonding | hydrogen
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| mnemonic for 3 elements that hydrogen must be bonded to for it to exert hydrogen bonding on neighboring molecules | FON
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| H-bonding causes water to _?_ when it freezes | expand
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| a(n) _?_ is an ionic compound with a set # of covalently-bonded water molecules attached to stabilize the crystal lattice | hydrate
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| describes the powdery part of a hydrate that remains when its water of hydration is removed, usually by heating | anhydrous
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| the • symbol in a hydrate formula (ex: CaCl₂•2H₂O) means "_?_ to" | attached
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| a covalent compound which, when dissolved in water, forms H⁺ ions and tastes sour | acid
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| the pattern "hydro-(root)-ic" ACID is used for an acid whose compound name ends in _?_ | ide
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| the pattern "(root)-ic" ACID is used for an acid whose compound name ends in _?_ | ate
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| the pattern "(root)-ous" ACID is used for an acid whose compound name ends in _?_ | ite
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| overall charge of a molecule | neutral
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| the BF₃ molecule violates the octet rule by having _?_ valence electrons around the central atom (B) | 6
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| the PCl₅ molecule violates the octet rule by having _?_ valence electrons around the central atom (P) | 10
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| the SF₆ molecule violates the octet rule by having _?_ valence electrons around the central atom (S) | 12
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| H-bonding holds together the 2 strands of the _?_ double helix | DNA
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| H-bonding can cause a(n) _?_ to fold so that it forms a 'receptor site' (Ex: hemoglobin forms a receptor site for O₂) | protein
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| when naming mixed compounds using Divide and Conquer, look for _?_ first | ammonium
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| when naming mixed compounds using Divide and Conquer (after dividing ammonium), you might use a Roman numeral if the first symbol is classified as a _?_ element | metal
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| when naming mixed compounds using Divide and Conquer (after dividing ammonium), you might use numerical prefixes (mono, di, etc) if the first symbol is classified as a _?_ element | nonmetal
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